Based only on intermolecular forces, which of the following compounds would be the least soluble in CH3OH?

• A. CH3COOH
• B. CCl4
• C. NH3
• D. H2O

Answer: (B)

Verified step by step guidance

1. Identify the type of intermolecular forces present in methanol (CH3OH). Methanol is a polar molecule capable of hydrogen bonding due to its -OH group.
2. Analyze the intermolecular forces in each compound: CH3COOH (acetic acid) can hydrogen bond and is polar; NH3 (ammonia) can hydrogen bond and is polar; H2O (water) can hydrogen bond and is highly polar; CCl4 (carbon tetrachloride) is nonpolar and exhibits only London dispersion forces.
3. Recall the principle 'like dissolves like,' meaning polar solvents dissolve polar solutes better, and nonpolar solvents dissolve nonpolar solutes better.
4. Compare the polarity and intermolecular forces of each compound to those of methanol. Since methanol is polar and hydrogen bonding, compounds that are also polar and can hydrogen bond will be more soluble.
5. Conclude that CCl4, being nonpolar and lacking hydrogen bonding, will have the weakest interactions with methanol and thus will be the least soluble among the given compounds.